Ch.9 - Molecular Geometry and Bonding Theories

Brown - Chemistry: The Central Science 14th Edition

Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook

Brown 14th Edition

Ch.9 - Molecular Geometry and Bonding Theories

Problem 100b

Chapter 9, Problem 100b

Sodium azide is a shock-sensitive compound that releases N2 upon physical impact. The compound is used in automobile airbags. The azide ion is N3-. (b) State the hybridization of the central N atom in the azide ion.

Verified step by step guidance

insert step 1> Identify the central atom in the azide ion (N3-).

insert step 2> Recognize that the azide ion is a linear molecule with the structure N-N-N.

insert step 3> Determine the number of regions of electron density around the central nitrogen atom.

insert step 4> Use the VSEPR theory to predict the hybridization based on the number of electron density regions.

insert step 5> Conclude the hybridization of the central nitrogen atom based on the linear geometry.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Hybridization

Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals can then be used to form covalent bonds in molecules. The type of hybridization depends on the number of electron pairs around the central atom, influencing the geometry and bonding properties of the molecule.

Azide Ion Structure

The azide ion (N3-) consists of three nitrogen atoms connected in a linear arrangement. The central nitrogen atom is bonded to two terminal nitrogen atoms, which can be represented as N=N^+=N^-. Understanding the structure of the azide ion is crucial for determining the hybridization of the central nitrogen atom, as it influences the distribution of electron density and bond angles.

Valence Bond Theory

Valence Bond Theory explains how atomic orbitals combine to form bonds in molecules. It emphasizes the role of electron pairs and the spatial orientation of orbitals. In the case of the azide ion, this theory helps in determining the hybridization state of the central nitrogen atom, which is essential for predicting the molecule's reactivity and stability.

Recommended video:

Guided course

00:47

Valence Shell Electron Pair Repulsion Theory

Related Practice

Textbook Question

Sodium azide is a shock-sensitive compound that releases N2 upon physical impact. The compound is used in automobile airbags. The azide ion is N3-. (a) Draw the Lewis structure of the azide ion that minimizes formal charge (it does not form a triangle). Is it linear or bent?

537

views

Textbook Question

a) Predict the electron-domain geometry around the central S atom in SF₂, SF₄, and SF₆.

701

views

Textbook Question

(b) The anion IO₄^- has a tetrahedral structure: three oxygen atoms form double bonds with the central iodine atom and one oxygen atom which carries a negative charge forms a single bond. Predict the molecular geometry of IO₆^5-.

Textbook Question

Butadiene, C4H6, is a planar molecule that has the following carbon–carbon bond lengths:

(a) Predict the bond angles around each of the carbon atoms and sketch the molecule.

1118

views

Textbook Question

In ozone, O3, the two oxygen atoms on the ends of the molecule are equivalent to one another. (d) How many electrons are delocalized in the p system of ozone?

1548

views